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Chapter 1 Dipoles, molecular polarity
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Ways to Represent Polarity in Molecules H F electron rich region electron poor region
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Dipole Moment ( ) H F electron rich region electron poor region = q x r magnitude of charge = = | | bond length moment in Debyes (D) 1 D = 3.36 x 10 -30 Coulomb. meter
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Explain the Trend EN drops
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More Complex Molecules? Consider molecular shape (bond orientation) bond polarity lone pairs (and sometimes) atom size What is symmetry of e- distribution?
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Consider NH 3 Lewis Structure Need # valence e- from all atoms Need bond arrangement (connectivity)
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Consider NH 3 Lewis Structure # valence e- = 5 (N) + 1 (3H) = 8e- Three N-H bonds H - N - H | H..
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Consider NH 3 From the Lewis structure Deduce e- pair geometry at central atom THEN find molecular geometry/shape Any predictions? H - N - H | H..
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: :: : Consider NH 3 molecular shape individual bond dipoles lone pair “dipoles” 4e- pairs at N tetrahedral e- pr geometry Lone pair at N molecular geometry/shape is trigonal pyramidal
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.. : :: : Which molecule is more polar? molecular shape individual bond dipoles lone pair “dipoles”
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.. : :: : Which molecule is more polar?
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.. : :: : Which molecule is more polar?
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Attractions Between Dipoles
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E coulomb q E coulomb 1/d
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Dipole-Dipole Interactions Dipoles align, + of one dipole to of another Magnitude of attraction E coulomb ( + )( )/d Increases with dipole moment ~5-25 kJ/mol …... d d
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NOFNOF H..…NOFNOF Hydrogen Bonding: Special Type of Dipole-Dipole Attraction From another molecule From one molecule Only applies to molecules with H bonded to N, O, or F ~10-40 kJ/mol (larger than most dipole-dipole attractions) ..… H bond
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Why Are Hydrogen Bonds So Strong? EN for H and N,O, F = very large, so N-H, O-H, F-H bonds are very polar ( + - are large) H atoms are small, so N, O, F of one molecule can closely approach H of another molecule (d is small) NOFNOF H … NOFNOF E coulomb ( + )( )/d H bond
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Hydrogen Bonds in Water
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Large Molecules Can Have Intramolecular Hydrogen Bonds
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Hydrogen Bonds in Chitin
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